Notice that in each case, the name is derived from the acid by replacing the "oic acid" ending by "amide".

If the chain was branched, the carbon in the -CONH2 group counts as the number 1 carbon atom. For example:

Physical properties

Melting points

Methanamide is a liquid at room temperature (melting point: 3°C), but the other amides are solid.

For example, ethanamide forms colourless deliquescent crystals with a melting point of 82°C. A deliquescent substance is one which picks up water from the atmosphere and dissolves in it. Ethanamide crystals nearly always look wet.

Note: Ethanamide is said to smell of mice. In fact, the smell is due to an impurity in the ethanamide called N-methylethanamide, CH3CONHCH3, where one of the hydrogens in the -NH2 group has been replaced by a methyl group.

The melting points of the amides are high for the size of the molecules because they can form hydrogen bonds. The hydrogen atoms in the -NH2 group are sufficiently positive to form a hydrogen bond with a lone pair on the oxygen atom of another molecule.

As you can see, there is the potential for lots of hydrogen bonds to be formed. Each molecule has two slightly positive hydrogen atoms and two lone pairs on the oxygen atom.

These hydrogen bonds need a reasonable amount of energy to break, and so the melting points of the amides are quite high.

Note: If you aren't happy about hydrogen bonding then you really ought to follow this link before you go on.

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Solubility in water

The small amides are soluble in water because they have the ability to hydrogen bond with the water molecules.

It needs energy to break the hydrogen bonds between amide molecules and between water molecules before they can mix - but enough energy is released again when the new hydrogen bonds are set up to allow this to happen.

Questions to test your understanding

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